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Calculate the pressure, in atmospheres, required to compress a sample of helium gas from 27.3 L (at 1.00 atm) to 3.36 L at constant temperature. Enter your answer in the box provided. atm

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sebassandin

Answer:

8.125 atm

Explanation:

Hello,

Boyle's law states that at constant temperature:

[tex]P_1V_1=P_2V_2[/tex]

In this case:

[tex]P_1=1 atm, V_1=27.3L, V_2=3.36L[/tex]

Solving for [tex]P_2[/tex]:

[tex]P_2=\frac{P_1V_1}{V_2}=\frac{1atm*27.3L}{3.36L}\\P_2=8.125atm[/tex]

Best regards!

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